Which of the following is the correct decreas | vedclass

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(C) $1$. The bond dissociation enthalpy generally decreases down the group due to an increase in atomic size and bond length.$2$. However, $F_2$ has a

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$Cl_2 > Br_2 > F_2 > I_2$

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(C) $1$. The bond dissociation enthalpy generally decreases down the group due to an increase in atomic size and bond length.$2$. However, $F_2$ has an exceptionally low bond dissociation enthalpy compared to $Cl_2$ and $Br_2$.$3$. This is due to the small size of the $F$ atom, which leads to strong inter-electronic repulsions between the non-bonding electrons of the two $F$ atoms in the $F-F$ bond.$4$. Therefore, the correct decreasing order is $Cl_2 > Br_2 > F_2 > I_2$.

Which of the following is the correct decreasing order of bond dissociation enthalpy of halogens?

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